Question

A compound contains only carbon, hydrogen, and oxygen. Combustion of 65.76 g of the compound yields 96.38 g of CO2 and 39.46 g of H2O.

The molar mass of the compound is 90.078 g/mol.
1. Calculate the grams of carbon (C) in 65.76 g of the compound:
2. Calculate the grams of hydrogen (H) in 65.76 g of the compound.
3. Calculate the grams of oxygen (O) in 65.76 g of the compound.

Answer 1

1. 26.30 g C.

2. 4.42 g H.

3. 35.04 g O.

Step-by-step explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to calculate the required as follows:

1. Here, the only source of carbon is in CO2, and thus, we calculate the grams of carbon from the produced grams of this substance:

`m_C=96.38gCO_2*(1molCO_2)/(44.01gCO_2) *(1molC)/(1molO_2) *(12.01gC)/(1molC) =26.30g`

2. Here, the only source of hydrogen is in H2O, and thus, we calculate the grams of hydrogen from the produced grams of this substance:

`m_H=39.46gH_2O*(1molH_2O)/(18.02gH_2O) *(2molH)/(1molH_2O) *(1.01gH)/(1molH) =4.42gH`

3. Here, we subtract the mass of H and C from the mass of the sample, to obtain the mass of oxygen:

`m_O=65.76g-26.30g-4.42g\\\\m_O=35.04g`

Regards!